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Difference between Internal Energy and Enthalpy

The value of ...

Question

The value of $(Δ H - Δ U)$ the formation of carbon monoxide from its elements at $298 K$ is:

- 2477.57 J m o l^{- 1}

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+ 2477.57 J m o l^{- 1}

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- 1238.78 J m o l^{- 1}

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+ 1238.78 J m o l^{- 1}

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Solution

The correct option is C $+ 1238.78 J m o l^{- 1}$
The reaction for the formation of carbon monoxide from its elements is given below:

$C (s) + \frac{1}{2} O_{2} (g) \to C O (g)$

Change in the number of moles $= Δ n_{g} = 1 - \frac{1}{2} = \frac{1}{2}$

$Δ H = Δ U + Δ n_{g} R T$

$∴ Δ H - Δ U = Δ n_{g} R T$ $= \frac{1}{2} R T$

$= \frac{1}{2} \times 8.314 \times 298$ $= 1238.786$ J/mol

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